At $300 \ K$,the following graph is obtained for one mole of an ideal gas. If its pressure is $10 \ atm$,then its volume (in $L$) will be

$A$ steel cylinder contains helium gas at $250 \, kPa$ pressure and $300 \, K$ temperature. The cylinder can withstand a maximum pressure of $1 \times 10^6 \, Pa$. The room in which the cylinder is placed catches fire. Predict whether the cylinder will burst before it melts. (Melting point of the cylinder = $1800 \, K$)

What will be the pressure exerted by a mixture of $3.2 \ g$ of methane and $4.4 \ g$ of carbon dioxide contained in a $9 \ dm^3$ flask at $27^{\circ} C$?

$A$ syringe has a volume of $10.0 \text{ cm}^3$ at a pressure of $1 \text{ atm}$. If the end is sealed and the plunger is pushed down at a constant temperature, what will be the final volume when the pressure becomes $3.5 \text{ atm}$ (in $\text{ cm}^3$)?

At what temperature in $K$ will $28 \ g$ of $N_2$ gas occupy a volume of $10.0 \ L$ at $2.46 \ atm$ pressure?

$A$ vessel contains $1.6 \ g$ of dioxygen at $STP$ ($273.15 \ K$,$1 \ atm$ pressure). The gas is now transferred to another vessel at constant temperature,where pressure becomes half of the original pressure. Calculate
$(A)$ volume of the new vessel.
$(B)$ number of molecules of dioxygen.